Ch.19 Equilibrium
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Homogeneous equilibrium
All species have same state
Heterogeneous equilibrium
Species are in different states
Kc with heterogeneous and homogeneous equilibriums
Homogeneous- all species Heterogeneous- solids and liquids omitted from Kc expression
Kc only includes what states
Aq and g
Process to find Kc
Equation React amounts Init mol Change Equilibrium mol
What is Kp
The equilibrium constant in terms of partial pressures Only gasses considered Omit any other states
Vol of gas and mols
Under same conditions the same vol of different gasses will contain the same number of moles
Mole fraction
The proportion by volume of a gas to the total volume of gasses in the mixture Mol of gas / total mols
Mole fractions of all gasses in a mixture =
1
Partial pressure (p)
Mole fraction of gas x total pressure
Sum of partial pressures =
Total pressure
Kp=
P(products) / p(reactants)
le chateliers principle rules
. if conc of species increases, eq position shifts in direction that reduces the conc . if pressure increases, the eq shifts towards side with fewer gaseous moles . if temp increased, eq shifts in endothermic direction
K=1
eq if at halfway point
K=100
eq is at products
K=0.01
eq is at reactants
when does K not change
at a set temp
when does K change
at different temps
K when increasing temp of exothermic reaction
decreases decreases product yield as it favours the reverse reaction so smaller product partial pressure smaller Kp
K when increasing temp of endothermic reaction
increases increases product yield as it favours the forward reaction so larger partial reassure of products larger Kp
what does a catalyst do to K
nothing catalysts affect the rate not the position of eq